When copper reacts with nitric acid, a mixture of NO(g) and NO2(g) is evolved. The volume ratio of the two product gases depends on the concentration of the nitric acid according to the equilibrium
Consider the following standard reduction potentials at 25°C:
a. Calculate the equilibrium constant for the above reaction.
b. What concentration of nitric acid will produce a NO and NO2 mixture with only 0.20% NO2 (by moles) at 25°C and 1.00 atm? Assume that no other gases are present and that the change in acid concentration can be neglected.
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Chemistry: An Atoms First Approach
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